How do isotopes differ in atomic structure?

Isotopes of an element have the same number of protons but different numbers of neutrons. This difference in neutron count leads to variations in their atomic masses. Here's a breakdown of their atomic structure differences:

Protons: Isotopes have the same number of protons, meaning they have the same atomic number and belong to the same element.
Neutrons: Isotopes differ in the number of neutrons. This difference results in different atomic masses for each isotope of the element.
Electrons: In neutral atoms, isotopes have the same number of electrons, ensuring they exhibit similar chemical properties.
Nucleus: The difference in neutron count leads to variations in the stability of the nucleus. Some isotopes may be stable, while others can be radioactive and decay over time.
For example, carbon has two common isotopes:

Carbon-12 (¹²C): 6 protons and 6 neutrons
Carbon-14 (¹⁴C): 6 protons and 8 neutrons
Despite having different atomic masses, both isotopes of carbon behave similarly in chemical reactions because they have the same number of protons and electrons.